Answered: Chemistry Question

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Step 1

When 5.00 moles of H₂ reacts with 5.00 moles of Cl₂ than 10 moles of HCl are formed. Therefore, the reaction can be written as:

$5 H_{2} (g) + 5 C l_{2} (g) \to 10 H C l (g)$

It is given that,

$\begin{array}{rcl} Δ H & = & - 184.6 k J / m o l \end{array}$

Since,

$Δ H = Δ U + Δ n_{g} R T . . . . . . . . . . (1)$

where

ΔH: Change in enthalpy (-184.6 kJ/mol).

ΔU: Change in internal energy.

Δn_g: Sum of moles of gaseous product – Sum of moles of gaseous reactant ({10 - [5+5] = 0}).

R: Gas Constant (8.314 JK^-1mol^-1).

T: Temperature (25 + 273 = 298^oC).

Step 2

Substituting all the values in equation (1) as-

$- 184.6 k J / m o l = Δ U + [0 \times 8.314 J K^{- 1} m o l^{- 1} \times 298 K] - 184.6 k J / m o l = Δ U + 0 Δ U = - 184.6 k J / m o l$

In kJ:

$\begin{array}{rcl} Δ U \times n & = & - 184.6 k J / m o l \times 5.00 m o l \\ = & - 923 k J \end{array}$

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